Multiple Choice
If Kc for the following reaction is 5.4 × 1013,
2 NO (g) + O2 (g) ⇆ 2 NO2 (g)
what is Kc for the reaction shown below?
4 NO2 (g) ⇆ 4 NO (g) + 2 O2 (g)
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16. Chemical Equilibrium
ICE Charts
Back16. Chemical Equilibrium
ICE Charts
- Multiple ChoiceCalculate the reaction quotient for the reaction below where the concentrations are [SO3] = 0.500 M, [SO2] = 0.0500 M, and [O2] = 0.100 M.
2 SO3 (g) ⇆ 2 SO2 (g) + O2 (g)
- Multiple ChoiceWhich of the following is a false statement about the relationship between Q and K?2views
- Multiple ChoiceA salt dissociates in water and can create an acidic or basic solution. Each ion of the salt can be hydrolyzed in water to form the corresponding acid or base. If the acid or base that forms is weak, what is the effect on the pH of the solution?
- Multiple Choice
For the reaction:N2 (g) + 2 O2 (g) ⇌ 2 NO2 (g), Kc = 8.3 x 10 -10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas?
- Multiple Choice
When 0.600 atm of NO2 was allowed to come to equilibrium the total pressure was 0.875 atm. Calculate the Kp of the reaction.
2 NO2 (g) ⇌ 2 NO (g) + O2 (g)
- Multiple ChoiceCalculate Kc for the following reaction at 300 K where the equilibrium concentrations are [SO3] = 0.400 M, [SO2] = 0.200 M, and [O2] = 0.600 M.
2 SO3 (g) ⇆ 2 SO2 (g) + O2 (g)
- Multiple Choice
Consider the following reaction:
COBr2 (g) ⇌ CO (g) + Br2 (g)
A reaction mixture initially contains 0.15 atm COBr2. Determine the equilibrium concentration of CO if Kp for the reaction at 25°C is 4.08.
- Multiple Choice
At a given temperature the gas phase reaction: N2 (g) + O2 (g) ⇄ 2 NO (g) has an equilibrium constant of 4.18 x 10-7. What will be the concentration of NO at equilibrium if 2.00 moles of nitrogen and 6.00 moles oxygen are allowed to come to equilibrium in a 2.0 L flask?
1views - Multiple ChoiceWhich of the following steps is essential when solving an ICE table for a chemical equilibrium problem?
- Multiple Choice
At a certain temperature, 0.810 mol NO is placed in a 5.00 L container. At equilibrium, 0.075 mol N2 is present. Calculate Kc.
2 NO (g) ⇌ N2 (g) + O2 (g)
- Multiple Choice
At a given temperature the gas phase reaction:N2 (g) + O2 (g) ⇌ 2 NO (g) has an equilibrium constant of 4.00 x 10 -15. What will be the concentration of NO at equilibrium if 2.00 moles of nitrogen and 6.00 moles oxygen are allowed to come to equilibrium in a 2.0 L flask.
- Multiple ChoiceThe following reaction has a Kc value of 4.1 × 10-31 at 25 ºC. Calculate Kp at this temperature.
N2 (g) + O2 (g) ⇆ 2 NO (g)